Defining the Trends
Atomic Radius
Electronegativity
Ionization Energy
A Little Bit of Everything
100
What happens to atomic radius as you go down the periodic table?
Atomic radius increases
100
Which atom is bigger: Sn or I?
Sn
100
Which atom is more likely to gain an electron: Y or Mo?
Mo
100
Which atom has higher ionization energy: Be or C?
C
100
Which atom is bigger: Be or C?
Be
200
What happens to electronegativity as you go across the periodic table?
Electronegativity increases
200
What atom is smaller: Ni or Ga?
Ga
200
Which atom is more likely to gain an electron: Se or Co?
Se
200
Which atom has lower ionization energy: H or Rb?
Rb
200
Which element has the lower electronegativity: Sn or I?
Sn
300
What happens to ionization energy as you go down the periodic table?
Ionization energy decreases
300
Which atom is bigger: Na or K?
K
300
Which atom is less likely to gain an electron: Cr or W?
W
300
Which atom is more likely to lose an electron: Cr or W?
W
300
Which atom is less likely to gain an electron: Te or O?
Te
400
As electronegativity decreases, an atom will become ______ likely to gain an electron.
less
400
Which atom is smaller: Tc or Mn?
Mn
400
Which element has the lower electronegativity: Mn or Re?
Re
400
Which atom is less likely to lose an electron: Sn or I?
I
400
Which atom is more likely to lose an electron: V or K?
K
500
If an atom has high ionization energy, is it more or less likely to lose an electron? Why?
Less likely because high ionization energy means it takes more energy to remove an electron, so it is less likely to happen.
500
Which atom is smaller: Se or Co?
Se
500
Which atom has the higher electronegativity: V or K?
V
500
Which atom is more likely to lose an electron: Te or In?
In
500
Which atom is less likely to lose an electron: Na or K?
Na
M
e
n
u